Electrical battery.



' PATENTED JUNE 14, 1904. J. R. LORD.

ELECTRICAL BATTERY.

APPLICATION rum) mus, 1003. N0 MODEL.

,W'ITNESSES V lNVENT -R:

. UNITED STATES PATENT I OFFICE.

Patented June 14, 1904.

7 JOHN" ROGER LORD, OF SAN FRANCISCO, CALIFORNIA.

ELECTRICAL BATTERY.

srn'cmrcn'rmn forming part of Letters Patent No. 762,425, dated June 14, 1904.

Application filed June 5, 1903. Serial No. 160,179. (No model.) i

To ail whom it may cor warn:

- Be itknown that I, J 01in ROGER LORD, a citizen of the United States, residing at San Fran cisco, California, have invented a new and useful Electrical Batterymf which the following is a specification.

My invention comprises a class of batteriesthe distinctive principle of which may be briefly stated thus: In any galvanic cell,-

whether employed as primary or secondary the anodeis chemically'attacked by-the electrolyte'and is hence diminishediin quantity,-

the active material of the anode combining with any or all/of the other elements of the battery, and when these reactions haveproceeded to a onclusion .thecell is said to be exhausted. n this invention the anode ac:

tive material is a compound of an anode metal.

The term anode metal is intended to mean any metal which'may be employed as an anode,-

. arrangement inthis battery are such that a.

compound of an anode metal is chemically -precipitated upon the anode from the used.

(that electrode i'rom which the "current or positive ion proceeds through the electrolyte in an electrically-active battery.)

The chemical combinationiand mechanical electrolyte, thereby vre-forming anode active material; The battery is hence regeneratory to this extent, yet While anode active material is automatically rev-formed in the cell other considerations, as will appear, cause the battery to gradually deteriorate in the course oftimean'd to ultimatelyrequire a process of "rehabilitation.

y Figure .1 inthe drawings illustrates a-form of galvanic cell, Abeing anode, E electrolyte,

and'K cathode.

' ode with and without solid depolarizer s.

Fig. 2 illustrates a form of anode; Figs; 3 and 4, different forms of oath..-

Fig. 5 represents aseries of cells similar to Fig. 1, or one cell divided into sections.-

Practically any known chemical combination for thechemical generation of an electrical current may with suitable mechanical arrangement .be made to automatically transform itself into the sort of regeneratory'element described.

reacts into Zn. ZnSO4+H2O C(Hz Whichescapes.)

.If the element is originally arranged as last shown, there is 'a current when circuit is closed, which, however, becomes rapidly polarized. If now the cathode beincreased in surface, the element remaining otherwise the same the'current is improved The cathode surface may be increasedby the employment of a finely-divided cathod'e metal. Theterm cathode metal. is intended to embrace any electrical conducting substance which may be employed as a cathode--in other .words, anysubstance the positive element of which is not chemically attacked by the electrolyte. The divisionmay be mechanical. or by precipitation. Constructionis illustrated in .Fig. .3, being the positive pole, F finely-divided conductors and P a porous en'- velop holding F in position if F is; of such characterias to require to be held.

stead of using Zn as an anode an oXidv of an anode metal is employed as anode active material the current is still further improved, the oxygen in the compound having a depolarizing eflect similar to that of a depolarizing agent difiused through the electrolyte or fixed at the cathode. The construction of an anode of this character is illustrated in Fig-2, where is the negative pole-piece connected to an extension of metal or other conducting material, upon which an oxid of an anode metal 0 is either placed. initially or precipitated by a subsequent chemical reaction in the electrolyte. It may be heated or baked or mixed with another compound to harden it and to thus improve the electrical connection. The conductor should preferably consist of a metal In the. element last above indicated if insimilar to that composing the oxid and should be placed in a horizontal position-at the bottom of theelectrolyte or at thebottom of any the anode. compound subsequently precipigood electrical results are had from this arrangement, it is found that the current is still further improved by providing an additional depolarizer at the cathode-such as CuO, PbOz, H2OI'O4, &c. the chemical action of whichis rendered apparently catalytic on account of the presence of a negative (or depolarizing) element in the active material of the anode; A depolarizing compound, which is insoluble in the electrolyte employed'is pref erable, though the diffusion of H2CIO4 or a similar solution through the electrolyte is not specially objectionable.

The theory Which follows is believed to explain the'operationof my battery and is based upon observed results. Arranged as above indicated the element is illustrated by anode electrolyte caithgde b 2 I ZnO znso.+n2o Cu If the cathode is merely finely-divided copper and 2110 is also omitted, it is observed that H2 evolves from the element if circuit stands closed for a time. The only hydrogen in the element is in H2O. Hence H2() is evidently decomposed.

When ZnSOi (or any other salt) is put into solution, there is a chemical reaction with water, as is evidenced by the thermal change. The rearrangement of moleculesjn the solution must be such that Zn can displace hydrogen, since .Zn does so. It is probably Zn from the anode may then displace H2, forming a structure thus:

agd releasing H2, which accumulates at catho e.

' When ZnO is employed as anode active ma terial, it is the Zn from ZnO which displaces H in the graphic structure, leaving the 0 from ZnO available to reoxidize the released H2, and thus obviating the necessity for Hz to draw on some other depolarizing agent.

The action of the additional depolarizer is' apparently catalytic. In support of this view are these facts: that the presence of such additional depolarizer very materially improves the character of the current, particularly with respect to the length of time it continues to be manifested, (a .matter of weeks,) with but slow deterioration in value on continuallyclosed circuit, and that after continued use of when first put into solution.

the battery such additional depolarizer is found not to have been reduced chemically. Its action may be and probably is this:

in which PbO2 (PbOO) is taken to be a depolariz'ing compound located at the cathode, H2

taken to represent the hydrogen displaced from the'electrolyte by Zn, (of Zn( and the escapes from the cell, and the PbO2 (or any equivalent depolarizer) is not reduced, where- .as in the absence of Zn() (or equivalent compound) as anode active material the Pb02 (or equivalent depolarizer) is reduced. Observe now that when Zn displaces H2 from the electrolyte the structure ZIIISIO4 O Zn is left suspended in water and that it, together with the unused zinc sulfate dissolved in water, constitute the electrolyte. It is immaterial which atom of -Zn attaches to O and which to theradical S04. It is ZnSOH-ZnO in water from any point of view; but while ZnSOi will remain in solution ZnO is not soluble in water nor in a solution of ZnSOi, and consequently the ZnO is precipitated. The ZnSO; with which it has been associated then decomposes 0r reassociates with another molecule of water in the same manner as It will be seen then that as much ZnO is precipitated upon the anode from the used electrolyte as is taken up from the anode in the displacement of H2 from solution structure in the electrolyte; but while this is the case there appears a gradual deterioration in the value of the current generated, due to other causes. One of them is that the fine precipitation falls upon the anode lightly and loosely and'makes a poor connection. This may be remedied at any time by pouring off the electrolyte and rebaking the anode to harden it into a solid mass. Another cause of deterioration in the current is that the cathode (or cathode depolarizer) becomes gradually filled in its intrieacies with an insoluble compound of the anode metal or of the metal which is in solution in the electrolyte. The insolubility of this compound is with respect to the electrolyte as a solvent under ordinary conditions. It may be dislodged by cleansing the cathode. This may be done with greater or less efficiency by heating it in the electrolyte, washing' it in water, or immersing it in an acid or other solution which will dissolve the undesirable accumulation of anode compound withresponding to the radical or negative ion con- I tained in the electrolyte) may be put into out afiecting the cathode metal or such depo larizing compound as may appertain to it.

For" example, PbOz (or its equivalent hardened vp asteqnade of Pb3Or+ Ht'SOQ'inay be cleansed with H2804. Cu ClzJor CuCh (as a depolarizer) will not be injuriously affected by HCL and so on. Such an acid-bath will removeany accumulation of anode-metal compounds not removable in water. In. case a porous pot or envelop is employed to con.- tain the cathode or cathode depolarizer an acid (preferably with a negative radical corsuch porous pot at cathode (K, Fig. 1) withoutdismantling the battery and with excellent results. Having followed these methods to an ultimate conclusion or until such a time as the resulting on rrent is no longer satisfactory, the whole battery may then be regenerated by any modification of the process described in my application, Serial No. 144,348, of February 20, 1903. A modification suggested is that since the electrolytevsolution haslittle orno commercial value it be thrown away and that merely the remaining, electrodes be treated, practically by the precess referred to. In experiments extendingover a year it has not yet been determined how much time must elapse before it becomes necessary to do this.

Having now described the principle upon which my invention is based, and which basicprinciple I claim to be new, there remains to call attention to the many chemical combinations by which the same results may be reached. For example, the element may be arranged as anode electrolyte gg s g 5Zn QHCl-HOHzO CT:

the plumbic sulfate being placed in the porous pot in the position of 'the depolarizer Fig. 4. The following reactions occur:

- zn+2Hc1=Zno1;+H..

- H2SO4lZn(anode) ZnSO4+ H2, which He escapes. The PbSO. has thus been reduced to finely-divided Pb, which is equivalent to the arrangement shown in Fig. 3. The element thus becomes 229 1 I I 3Zn -l-TOHzO GU which, in other words, is

I Zn' SO4 ,Zn Cl2 and on closed circuit becomes .Z l I (H2 escap- Zn Cu which on precipitation of '2ZnO is manifestly identical with the battery just described. Each anode salt ZnOlt' and ZnSOi operates independently in the same solution. Either of them will generate a current, and any number ofsimilar salts may be employed in this Lparallel manner in the same cell.

As one other example. of self-transformation let anelementbemarranged as anode electrolyte cathode -3Zn H.so.+H.o 3

Then

Zn+H2SOi=ZnSOl+Ha which is again the original proposition. Elements containing an alkaline metal in the electrolyte amount to practically the same thing.

The term alkaline metal is meant to embrace all of,those metals which decompose waterinto. a hydrate, such as sodium, calcium, ammonium &c.

' Let anelement be arranged as which is the simplest and most direct method of putting it together.

When K2804 is put into solution, there is 1 an endothermic manifestationindication, a rearrangement of atoms between it and Water slmilar to that between water and ZnSOi. The structure may begin in the same manner, thus:

SOiH2 but the upper part (K20) also reacts with watraiiil'nfilyuuidio the structure thu In any ordinary battery employing an alkaline hydroxld foran electrolyte such electrolyte when fully used or exhausted consists of an acidic salt, such 381(2241102, the anode metal filling the part of a negative radical. If KgZnOg be added to ZnSOi in solution, ZnO is precipitated, the reaction being ZI1S04 I QZI'IO,

and the element. thu's returns to its original chemical constituency, (minus incidental exceptions noted.) There is, however, an additional consideration in connection with this cell in that ZN(OH)2 is observed to be also precipitated on the anode and to act as additional anode active material The reactions given represent one set of molecules; but while IQZnOZ and ZnSOi are forming in the electrolyte the electrolyte also contains, of course, a quantity of the original K280i, which in the course of its reactions involves the temporary formation of QKOH, as shown. Then as an additional ramification the first line of the first gralic form (QKOH) and the last line of the second form '(ZnSOi) reacttogether thus:

which latter is precipitated to the anode. The precipitated Zn(Ol-l)3 then performs the function of anode active material in precisely the same manner that ZnO would:

r s oi o n;

l\' -SOi t i l.

It is understood, of course, that the exam ples employed are intended to represent a class, and that in reaching the resultsdescribed the individual chemical components which maybe substitued are practically innumerable.

Any combination of chemicals comprising a battery which by reason of their own chemical reaction finally become transformed into practically the same thing "as the battery described is manifestly equivalent thereto.

It should be borne in mind that the battery herein proposed generates an electrical current and that in order for it to do so there must necessarily be chemical reaction. reactionsdescribed occur only on closed circuit, and the galvanic circuit is apparently the cause of theirbccurring. When the'circuit is open, the'elements fall back to their normal state, minus such deteriorating changes as have been already mentioned.

It is observed in thisbattery that after it has been continuously at work for a time (varying from some days to some weeks, according to its structure) and the value of the current has decreased a very decided recovery in the value of the current is had by allowing the battery to stand on open circuit. This is probably due to the fact that the closed circuit induces the reaction which takes up the,

active material of the anode. It is evident that the longer the battery is at work the more anode material will be in suspension, solution,

or combination with the electrolyte and the less capable will the electrolyte be of taking up more, whereas when the circuit is open no more anode material is taken up and that which is alreadysuspended in the electrolyte is precipitated. It is obvious that the effect of thus clearing the electrolyte is essentially regeneratory in character. It is also observed that after the battery has been some time at work, with a gradual decrease in the value of the current as above, a marked improvement is bad by heating the whole battery. The efiect is probably due in chief measure to three points: first, that a raised temperature im- The 1 IIO proves the capabilities of water as a solvent of solids, stimulating and sharpening the so lution structure of the electrolyte; next, that the heating tends to settle or rearrange the position of the active material which has previously been precipitated from the electrolyte and puts it into firmer contact with the anode; finally, that the heating of the electrolyte dissolves or dislodges a part of any accumulated anode compounds which may have found a lodgment in the intricacies of the cathode.

As may be inferred, the degree of regeneraprecise construction shown in the drawings.

' An, 1 mechanical arran ement of partsma be 1 employed which does v tialprinciples.-

not interfere with essen- I claim.

1. An electricalbattery having an anode composed of an electrical conductor upon or around which is placed or deposited'a quantity of a compound ofan anode metal; such conductor serving as negative pole and beingplaced in such position that any solids chem 'ically precipitated from the electrolyte may fall in proximity thereto; such solids thereby forming anode active material: havingan' electrolyte composed of one or more'salts of one or'more anode metals in solution; and having a cathode'composed of any conducting substance chemically unattached by the electrolyte; substantially as described.

2. An electrical battery having an anode composed of an electrical conductor upon or.

around'whichis placed or deposited a quan'.

tity of a compound of an anode metal; such conductor serving. as negative pole and being placed in such position that any solids chemically precipitated fromithe'electrolyte may i fall in proximity thereto; such solids thereby forming anode active material; having an electrolyte composed of one or more salts of one or'more anode metals in solution: having any suitable compound in the position of de polarizer; and having a cathode composed of any conducting substance chemically unattackcd by the electrolyte;substantially as described.

3. An electrical batteryhaving ananode composed of an electrical conductor upon or around which is placed or deposited a quantity of a-compound of an anode metal; such conductor'serviug as negative pole and being placed in such position that any solids chemically precipitated from the electrolyte may fall in prox- 'imity thereto; such solids thereby forming anode active material; having an electrolyte composed of one or more salts of one or more alkaline metals in vsolution; and having a cathode composed of any conducting substance chemically unattacked by the electrolyte; substantially as described.

4. An electrical battery having an anode composed of an electrical conductor upon or around which is placed or deposited a quantity of acompound of an anode metal; such conductor serving as negative pole and being placed in such position that any solids chemically precipitated from the electrolyte may fall in proximity thereto; such. solids thereby forming anode activematerial: having an electrolyte composed of one or more salts of one or more alkaline metals in solution: having any suitanode active material: having an electrolyte composed of one'or moresalts of one or more anode metals together with one or more salts 'of one or more alkaline metals insolution; and

having a cathode composed of any conducting substance chemically unattached by the electrolyte; suhstantially as described, Y

6. An electrical battery having an anode composed of an electrical conductor upon or around which is-placed or deposited a quantity of compound of an anode i; such conductor servin as negative pole ansv being placed in such position that any solids chemically precipitated from the electrolyte may fall in proximity thereto; such solids thereby forming anode active material: having an electrolyte composed of one or more salts of one or more anode metals together with one or more salts of one or more alkaline metals in solution; having any suitable compound in the position of .depolarizer; and having" a cathode composed of any conducting substance chemically unattached by the electrolyte; substantially as de scribed 7. An electrical battery consisting of an anode, electrolyte and cathode in a containing vessel; the anode thereof being placed in such position in the electrolyte that any solids chemically precipitated from such electrolyte may 'fall upon or in electrical proximity to such anode; such precipitated solids thereby forming additional anode active material; substantially as described.

8. An electrical battery consisting oi an anode, clecti'olyte, depolarlzer and cathode 1n a containing vessei; anode thereof being placed in such position. in the electrolyte that any solids chemically precipitated from such electrolyte may fall upon or in electrical pro imity to such anode; such precipitated solids thereby forming additional anode active material; substantially as described.

9. In an electrical battery the combination of an electrolyte of metallic salts in solution a suitable compound in the position of depolarizer, and an anode formed by fixing into electrical contact with a conductor serving as negative pole, the compound or compounds precipitated from the electrolyte during previous use of the battery; substantially as described.

10 In an electrical battery the combination pounds precipitated from the electrolyte during previous use of the battery, for the purpose of again precipitating a solid to be thereafter utilized as anode active material; substantially as described.

11. In an electrical battery, an anode formed '10 by fixing into electrical contact with a conductor serving as negative pole, the compound or compounds of anode metal, formed and pre- I In testimony whereof I have signed my name '5 in the presence of two subscribing Witnesses.

J. ROGER LORD.

Nitnesses:

Jonn Boss, M. J. REEVES. 

